Ch.13 - Chemical KineticsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: The rate constant for the decomposition of N 2O(g) is 1.1×10−3 M-1 sec-1. Assuming that the initial concentration of N2O(g) is 0.2M, which of the following statements is true? a) The reaction is zero

Problem

The rate constant for the decomposition of N 2O(g) is 1.1×10−3 M-1 sec-1. Assuming that the initial concentration of N2O(g) is 0.2M, which of the following statements is true?

a) The reaction is zeroth order and the half life is 90.9 seconds

b) The reaction is first order and the half life is 90.9 seconds

c) The reaction is first order and the half life is 630 seconds

d) The reaction is second order and the half life is 4545.5 seconds

e) The reaction is second order and the half life is 630 seconds